The solubility of $AgCl$ in $0.2 \ M \ NaCl$ solution ($K_{sp}$ for $AgCl = 1.20 \times 10^{-10}$) is:

If the solubility product of $PbS$ is $8 \times 10^{-28}$,then the solubility of $PbS$ in pure water at $298 \ K$ is $x \times 10^{-16} \ mol \ L^{-1}$. The value of $x$ is $\dots$.
[Given $\sqrt{2} = 1.41$]

The solubility product constants of $M(OH)_3$ and $M(OH)_2$ are $10^{-23}$ and $10^{-14}$ respectively. If both ions are present in a solution,which one will precipitate first upon the addition of $NH_4OH$?

If the solubility product of $CaSO_4$ is $2.5 \times 10^{-5}$,then its solubility will be .......

At $T(K)$,$K_{sp}$ of two ionic salts $MX_2$ and $MX$ is $5 \times 10^{-13}$ and $1.6 \times 10^{-11}$ respectively. The ratio of molar solubility of $MX_2$ and $MX$ is

Precipitation occurs if the ionic product is ........